AP Chemistry Review Questions - Liquids and Solids

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The correct order for increasing boiling point among the noble gases is:

1. He
2. Ne
3. Ar
4. Kr
5. Xe

This phenomenon is best explained in terms of:
1. hydrogen bonding
2. covalent bonding
3. dipole-dipole interaction
4. Hund's rule
5. London dispersion forces
Which of the following statements is false?

1. Liquids with large intermolecular forces tend to have very low boiling points
2. Liquids with large intermolecular forces tend to have considerable surface tension
3. When a substance changes from a solid to a liquid, the molecules remain intact
4. The hardness of diamond is due to strong dipole-dipole attraction
1. 1 and 4
2. 2 and 3
3. 2 and 4
4. 3 and 4
5. 1 and 3
A metal has crystallized with a face-centered cubic lattice. The edge of the unit cell is 366 pm. What is the diameter of the metal atom?
1. 3.98 x 10^-5 pm
2. 518 pm
3. 259 pm
4. 267912 pm
5. 0.0296 pm
Which of the following hydrocarbons has the highest boiling point?
1. These are all gases and do not boil
2. C₄H₁₀
3. CH₄
4. C₂H₆
5. C₃H₈
Buckminsterfullerene is one of the allotropic forms of:
1. oxygen
2. carbon
3. steel
4. silicon
5. semimetals
The triple point of compound X occurs at a temperature of:
1. 50°C
2. 23°C
3. 29°C
4. -10°C
5. 80°C
The triple point of CO₂ is 5.2 atm and -57°C. In a laboratory at EDHS, on a day when the pressure is 758 torr and the temperature in the room is 20°C, a solid sample of carbon dioxide will:
1. remain solid
2. melt
3. sublime
4. boil
5. freeze
Which of the following is not an endothermic process?
1. sublimation
2. combustion
3. crystallization
4. vaporization
5. melting
Which of the following substances will have the greatest vapor pressure at 0°C?
1. NaCl
2. CH₄
3. H₂O and NH₃
4. NH₃
5. H₂O
The only intermolecular forces existing between oxygen molecules are:
1. nuclear forces
2. permanent dipole forces
3. ion-ion attractive forces
4. hydrogen bonding forces
5. London dispersion forces
How much energy is needed to convert 50.0 g of ice at -5.00°C to water at 25°C?
- Specific heat(ice) = 2.10 J/(g°C)
- Specific heat(water) = 4.18 J/(g°C)
- Heat of fusion = 333 J/g
- Heat of vaporization = 2258 J/g
1. 18.0 J
2. 175 J
3. 21.9 kJ
4. 37.3 kJ
5. 22.4 kJ
The normal boiling point of X is most likely:
1. 28°C
2. 80°C
3. 22°C
4. 50°C
5. 90°C
Place the following in order of increasing strength:

1. hydrogen bonding
2. covalent bonding
3. London dispersion forces
1. 1, 3, 2
2. 3, 1, 2
3. 2, 1, 3
4. 1, 2, 3
5. 3, 2, 1
An example of an amorphous solid is:
1. plastic
2. gold
3. ice
4. diamond
5. quartz
As the pressure increases, the melting point of compound X will:
1. increase and then decrease
2. decrease and then increase
3. decrease
4. stay the same
5. increase
For a solution in a closed container at equilibrium, which of the following pairs represent processes that must be occuring at equal rates?
1. evaporation and condensation
2. evaporation and sublimation
3. fusion and boiling
4. crystallization and sublimation
5. evaporation and crystallization
At a pressure of 1.3 atm and 20°C, compound X exists as:
1. a solid only
2. a liquid and a gas
3. a solid and a gas
4. a solid and a liquid
5. a liquid only